Chemists use stoichiometry in industry to determine quantities of chemicals needed, and to predict quantities of product, in any given useful chemical reaction. Without stoichiometry, industrial chemistry would be impossible, and we would live without most of the technological benefits to which we have become accustomed. Your group's task is to design a chemical reaction, and determine quantities required, for an industrial application. You will need to research the appropriate reactions, balance the reaction equation, and determine the amount of reactants needed to make the desired amount of product.
Your group works for Chalk, Incorporated, which supplies calcium oxide to coal-fired power plants. Chalk, Incorporated, uses limestone as its only raw material to make the calcium oxide. The calcium oxide then reacts with carbon dioxide, in the stacks of coal-fired power plants, which makes the limestone back again. The limestone also reacts with sulfur dioxide in the stacks of a coal-fired power plant in Cumberland City, Tennessee. The end product of that reaction is gypsum, which Chalk, Incorporated trucks from the power plant and sells to a wallboard manufacturer.
Group Your group will be divided into one of 3 roles.
Recorder - This person records the activities, writes on the lab report and updates the group website. This person also acts as the judge for all disagreements.
Calcium Oxide Manager - This person is responsible for all aspects of the production of Calcium Oxide. Research the chemical reaction needed to make calcium oxide from limestone, using the resources below. Devise a balanced chemical equation for the reaction.
Gypsum Products Manager - This person is responsible for all aspects of the production of Gypsum products. Research the chemical reactions needed to make gypsum from calcium carbonate and sulfur dioxide, using the resources below. Devise a balanced chemical equation for the reaction.
Task
Determine formulas for all of the reactants and products for all of the reactions.
Determine the equation for the combustion of carbon (coal).
Determine the equation for the combustion of sulfur.
Determine the equation for the combustion of nitrogen to form nitrogen dioxide.
Determine the equation for the combination of calcium oxide and water to form calcium hydroxide.
Determine the equation for the production of gypsum from sulfur dioxide and calcium hydroxide.
Determine the equation for the production of calcium oxide from limestone.
Predict the amount of gypsum would be produced from 50.0 g of calcium oxide and sulfuric acid (H2SO4). We will be using sulfuric acid because it is easier to handle and less hazardous than sulfur dioxide.
Design an experiment and write a procedure for testing your prediction above. Your experiment must be approved by your teacher.
Follow your procedure. Calculate your yield, and percent yield.
Determine how many tons of calcium oxide you would need to remove 1.00 ton of sulfur dioxide. From this, also determine how many tons of gypsum can be made from the same reaction.
The percent composition of a load of coal is given below. If 1 ton of coal is burned, how many tons of carbon dioxide are produced? How many tons of water is produced?
If 1.00 ton of coal is burned, how many tons of sulfur dioxide is produced?
If 1.00 ton of coal is burned, how many tons of nitrogen dioxide is produced?
If 1.00 ton of coal is burned, how many tons of calcium oxide is required to sequester the carbon dioxide produced?
If 1.00 ton of coal is burned, how many tons of gypsum can be produced?
EXTRA CREDIT : Determine market values for limestone, calcium oxide, sulfuric acid and gypsum. Be sure to cite your sources.
Along with your lab sheet, you will hand in a completed Grading Rubric. This is your self evaluation. Mr. Haugen will also fill out a Grading Rubric on your performance, and the two grades will be added together.
Coal Plant Webquest
Introduction
Chemists use stoichiometry in industry to determine quantities of chemicals needed, and to predict quantities of product, in any given useful chemical reaction. Without stoichiometry, industrial chemistry would be impossible, and we would live without most of the technological benefits to which we have become accustomed.Your group's task is to design a chemical reaction, and determine quantities required, for an industrial application. You will need to research the appropriate reactions, balance the reaction equation, and determine the amount of reactants needed to make the desired amount of product.
Your group works for Chalk, Incorporated, which supplies calcium oxide to coal-fired power plants. Chalk, Incorporated, uses limestone as its only raw material to make the calcium oxide. The calcium oxide then reacts with carbon dioxide, in the stacks of coal-fired power plants, which makes the limestone back again. The limestone also reacts with sulfur dioxide in the stacks of a coal-fired power plant in Cumberland City, Tennessee. The end product of that reaction is gypsum, which Chalk, Incorporated trucks from the power plant and sells to a wallboard manufacturer.
Group
Your group will be divided into one of 3 roles.
Recorder - This person records the activities, writes on the lab report and updates the group website. This person also acts as the judge for all disagreements.
Calcium Oxide Manager - This person is responsible for all aspects of the production of Calcium Oxide. Research the chemical reaction needed to make calcium oxide from limestone, using the resources below. Devise a balanced chemical equation for the reaction.
Gypsum Products Manager - This person is responsible for all aspects of the production of Gypsum products. Research the chemical reactions needed to make gypsum from calcium carbonate and sulfur dioxide, using the resources below. Devise a balanced chemical equation for the reaction.
Task
- Determine formulas for all of the reactants and products for all of the reactions.
- Determine the equation for the combustion of carbon (coal).
- Determine the equation for the combustion of sulfur.
- Determine the equation for the combustion of nitrogen to form nitrogen dioxide.
- Determine the equation for the combination of calcium oxide and water to form calcium hydroxide.
- Determine the equation for the production of gypsum from sulfur dioxide and calcium hydroxide.
- Determine the equation for the production of calcium oxide from limestone.
- Predict the amount of gypsum would be produced from 50.0 g of calcium oxide and sulfuric acid (H2SO4). We will be using sulfuric acid because it is easier to handle and less hazardous than sulfur dioxide.
- Design an experiment and write a procedure for testing your prediction above. Your experiment must be approved by your teacher.
- Follow your procedure. Calculate your yield, and percent yield.
- Determine how many tons of calcium oxide you would need to remove 1.00 ton of sulfur dioxide. From this, also determine how many tons of gypsum can be made from the same reaction.
- The percent composition of a load of coal is given below. If 1 ton of coal is burned, how many tons of carbon dioxide are produced? How many tons of water is produced?
- If 1.00 ton of coal is burned, how many tons of sulfur dioxide is produced?
- If 1.00 ton of coal is burned, how many tons of nitrogen dioxide is produced?
- If 1.00 ton of coal is burned, how many tons of calcium oxide is required to sequester the carbon dioxide produced?
- If 1.00 ton of coal is burned, how many tons of gypsum can be produced?
EXTRA CREDIT : Determine market values for limestone, calcium oxide, sulfuric acid and gypsum. Be sure to cite your sources.----
Resources
Capturing CO2
Capturing SO2
Patent on SO2
Gypsum
Limestone
Coal Plant
All About Coal
Coal Composition
Grading
Along with your lab sheet, you will hand in a completed Grading Rubric. This is your self evaluation. Mr. Haugen will also fill out a Grading Rubric on your performance, and the two grades will be added together.Credits
This webquest is based upon another webquest created by Rebecca M. Turner at the Nashville School of the Arts, located here.